NO$2($g$)+$ CO$($g$)-->$ NO$($g$)+$ CO$2($g$)$

The rate of the above reaction depends only on the concentration of nitrogen dioxide at temperatures below $225\backslash$deg C$.$

At a temperature below $225\backslash$deg C the following data were obtained:

Time

$($s$)$

$[$NO$2]$

$($mol$/$L$)$

$0$

$0\mathrm{.}580$

$8\mathrm{.}00\backslash$times $102$

$0\mathrm{.}552$

$2\mathrm{.}00\backslash$times $103$

$0\mathrm{.}515$

$3\mathrm{.}00\backslash$times $103$

$0\mathrm{.}488$

$6\mathrm{.}00\backslash$times $103$

$0\mathrm{.}422$

$1\mathrm{.}20\backslash$times $104$

$0\mathrm{.}331$

Which of the following expressions for the rate law $($either differential or integrated$)$ are completely consistent with the above experimental data.

ln$[$NO$2]-$ ln$[$NO$2]0=-$kt

$-$d$[$NO$2]/$dt $=$ k

$1/[$NO$2]-1/[$NO$2]0=$ kt

k$[$NO$2]2=-$d$[$NO$2]/$dt

$[$NO$2]=[$NO$2]0-$ kt